Home
Class 11
CHEMISTRY
Calculate pH of 1 M PO4^-3) (aq) solutio...

Calculate pH of `1 M PO_4^-3)` (aq) solution.
`pk_b(PO_4^-3) = 1.62`

Promotional Banner

Topper's Solved these Questions

  • ENVIRONMENTAL CHEMISTRY

    PATHFINDER|Exercise QUESTION BANK|157 Videos
  • GOC-II & III

    PATHFINDER|Exercise QUESTION BANK|144 Videos

Similar Questions

Explore conceptually related problems

Calculate the pH of 0.05 (M) H_(2) SO_(4) solution .

To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100mL of 0.1 M acetic acid solution [ pkb (CH3COO-)=9.26] is:

Calculate the concentrations of Ca^(2+) and PO_4^(3-) ions in a saturated [Ca_3(PO_4)_2] solution. Given: K_(sp)[Ca_3(PO_4)_2]=2.0xx10^(-29) (at 25^(@)C )

At what concentration of PO_(4)^(3-) ions in 0.1(M) aqueous solution of AgNO_(3), will Ag_(3)PO_(4) start to precipitate?Given: K_(sp)(Ag_(3)PO_(4))=1.3xx10^(-20) .

The degree of ionisation of a 0.1(M) bromoacetic acid solution is 0.132. calculate the pH of the solution and the pK_(a) of bromoacetic acid.

Charge carried by 1 mole PO_4^(3-) ions is.

pH of 0.05(M) calcium acetate solution (pK_a=4.74) is -

PATHFINDER-EQUILIBRIUM-QUESTION BANK
  1. The pH of a buffer is 4.745. When 0.01 mol of NaOH is added to 1 litre...

    Text Solution

    |

  2. Calculate the pH of the solution in which 0.2M NH4CI and 0.1 M NH3 are...

    Text Solution

    |

  3. Calculate pH of 1 M PO4^-3) (aq) solution. pkb(PO4^-3) = 1.62

    Text Solution

    |

  4. Hydrolysis constant of NH4^+ is 5.55 xx 10^(-10). What is ionisation c...

    Text Solution

    |

  5. A weak acid HX has the dissociation constant 1xx10^-5M. It forms a sal...

    Text Solution

    |

  6. The solubility product of Mg (OH)2 is 1×10^(−11). At what pH, precipit...

    Text Solution

    |

  7. If a saturated solution is prepared by dissolving Ag2CO3 in water has ...

    Text Solution

    |

  8. Calculate the solubility of A2X3 in pure water, assuming that neither ...

    Text Solution

    |

  9. Calculate the molar solubility of Ni(OH)2 in 0.10 M NaOH. The solubili...

    Text Solution

    |

  10. An indicator has pkin = 5.3. In a certain solution, this indicator is ...

    Text Solution

    |

  11. An indicator has pkin = 5.3. In a certain solution, this indicator is ...

    Text Solution

    |

  12. The ionization constant of an acid-base indicator (a weak acid) is 1.0...

    Text Solution

    |

  13. Calculate the degree of ionization of 0.1 M acetic acid. The dissociat...

    Text Solution

    |

  14. Calculate the concentration of OH^ ions of 0.01 M NH4OH : Kb = 1.58 xx...

    Text Solution

    |

  15. At 15^@C 0.05 N solution of a weak monobasic acid is 3.5% ionised. Cal...

    Text Solution

    |

  16. Calculate ka for a dibasic acid if its concentration is 0.05 N and hyd...

    Text Solution

    |

  17. Calculate the approximate pH of 0.1 M aqueous H2S solution. K1 and k2 ...

    Text Solution

    |

  18. 9.8 g of H2SO4 is present in 500 mL of the solution. Calculate the pH ...

    Text Solution

    |

  19. Find the concentration of H^+, HCO3^-, and CO3^(2-) in a 0.01 M soluti...

    Text Solution

    |

  20. The degree of dissociation of water is 1.8 xx 10^(-9) at 298 K. Calcul...

    Text Solution

    |